When drinking through a straw, you are able to control the height of the liquid inside the straw by changing the pressure inside your mouth, as shown in the figure. What happens if the pressure in your mouth is lower than the air pressure outside? O Your mouth pressure will force the liquid down through the straw. O The outside air pressure will force the liquid up the straw and into your mouth. The liquid in the straw does not move. O The outside air pressure will force the liquid down the straw.

Suppose a student repeated Lab 1 using a different divalent metal X. The molar mass of metal X is 43.8 g/mol. An unknown mass of metal X was reacted with excess HCI (1 mole of Metal X produces 1 mole of H2 gas). The volume of H, gas produced was 26.53 mL. The reaction was performed at an atmospheric pressure of 547.6 mm Hg and at 18.0 °C. Calculate the mass of metal X that was used in the reaction. (Ignore the water vapour pressure (pH,O)) L-mm Hg R=62.4 7mol-K Answer:

A mixture of two gases (gas X and gas Z) is pumped into a sealed container half-way filled with 5.0 L of water. The total pressure of the gases over the water is 1.34 atm. If the pressure of gas Z is 0.52 atm. How many grams of gas X are in the water if the molar mass for gas X is 22.31 g/mol? The Henry's law constant for gas X is 0.0266 mol/(L-atm). 16. Grams of gas X:

A SCUBA driver is 100 ft below the surface of the ocean where the water exerts a pressure 43.3 psi at 18.0o The diver exhales and many bubbles are released and these bubbles rise to the surface where the atmospheric pressure is 1.03 psi and the temperature is 36.0o C.  One bubble has a volume of 20.0 mL.  What is the volume of the bubble at the surface?  You may assume the composition of the bubble does not change and the bubble remains intact as it rises.   P1 =                              P2 = V1 =                              V2 = n1 =                              n2 = T1 =                               T2 =

A sample of air from a home is found to contain 4.3×10−6 ppm of carbon monoxide. This means that if the total pressure is 735 torr, then the partial pressure of CO is ________ torr.

Oo.140. Subject:- Chemistry

Imagine that unknown gas in the storage tank is analyzed. A 14.74-g sample of the gas contains 9.97 g N2, 1.39 g CH4 , and 2.65 g CO2. Calculate the partial pressures of each gas (in bar) in the storage tank if the total pressure in the tank is 3.15 bar.

A balloon of volume 100.2 L contains a gas at a temperature of 22.0°C and pressure of 0.981 atm. This balloon is released, travels upward in the atmosphere, and passes over the top of Pikes Peak. At the top of Pikes Peak the temperature is 1.24°C and the balloon has expanded to 144.5 L. What is the pressure of the gas inside the balloon as as it clears the top of America’s Mountain?